Chemistry: Atoms First
2nd Edition
ISBN: 9780073511184
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 14, Problem 14.42QP
A student placed 1 g of each of three compounds A, B, and C in a container and found that after 1 week no change had occurred. Offer some possible explanations for the fact that no reactions took place. Assume that A, B, and C are totally miscible liquids.
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Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc for the
initial set reaction conditions in a 2.00 L container:
0.0560 g H2, 4.36 g l2, and 1.32 g HI.
H:(g) + lz(g) = 2 HI(g)
Based on the given data, set up the expression for Qc and then evaluate it. Do not combine or simplify terms.
Qc
=
The process
2XO₂(g) + O₂(g) = 2XO3(g)
is known to be endothermic. If a gas chamber containing an equilibrium
mixture is heated, then
XO3 would be produced. This is because
in this process.
heat can be considered one of the
B
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more, reactants
more, products
less, reactants
less, products
О А ОВ.О C O D
13. For the reaction,
250, (g) + O, (g) 2 250, (g), K, = 9 x 102
at 800 K, and K. = 1 x 106 at 635 K. Which of the
following is wrong about this reaction?
A) It is an exothermic reaction.
B) AL 800 K, SO, molecules are more stable than
those at 635 K.
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C) The heat content of SO, molecules is less than
that of SO, molecules.
D) K, is smaller than Ke at 800 K.
E) The rátio of specific rate constant for forward re-
action to that of the reverse reactión at 635 K is
Ix10
Chapter 14 Solutions
Chemistry: Atoms First
Ch. 14.3 - Determine the change in entropy for 1.0 mole of an...Ch. 14.3 - Determine the change in entropy (Ssys) for the...Ch. 14.3 - To what fraction of its original volume must a...Ch. 14.3 - From the standard entropy values in Appendix 2,...Ch. 14.3 - Prob. 2PPACh. 14.3 - In each of the following reactions, there is one...Ch. 14.3 - For each reaction shown in the diagrams, indicate...Ch. 14.3 - For each process, determine the sign of S for the...Ch. 14.3 - Prob. 3PPACh. 14.3 - Make a qualitative prediction of the sign of Hsoln...
Ch. 14.3 - Consider the gas-phase reaction of A2 (blue) and...Ch. 14.3 - Prob. 14.3.1SRCh. 14.3 - Prob. 14.3.2SRCh. 14.3 - Prob. 14.3.3SRCh. 14.4 - Determine if each of the following is a...Ch. 14.4 - For each of the following, calculate Suniv and...Ch. 14.4 - (a) Calculate Suniv and determine if the reaction...Ch. 14.4 - The following table shows the signs of Ssys,...Ch. 14.4 - Prob. 14.4.1SRCh. 14.4 - Prob. 14.4.2SRCh. 14.4 - Prob. 14.4.3SRCh. 14.5 - According to Table 14 4, a reaction will be...Ch. 14.5 - A reaction will be spontaneous only at low...Ch. 14.5 - Given that the reaction 4Fe(s) + 3O2(g) + 6H2O(l) ...Ch. 14.5 - Prob. 5PPCCh. 14.5 - Prob. 14.6WECh. 14.5 - Prob. 6PPACh. 14.5 - For each reaction, determine the value of Gf that...Ch. 14.5 - Prob. 6PPCCh. 14.5 - Prob. 14.7WECh. 14.5 - Prob. 7PPACh. 14.5 - Prob. 7PPBCh. 14.5 - Prob. 7PPCCh. 14.5 - Prob. 14.5.1SRCh. 14.5 - Prob. 14.5.2SRCh. 14.5 - Prob. 14.5.3SRCh. 14 - Explain what is meant by a spontaneous process....Ch. 14 - Which of the following processes are spontaneous...Ch. 14 - Prob. 14.3QPCh. 14 - Prob. 14.4QPCh. 14 - Prob. 14.5QPCh. 14 - Prob. 14.6QPCh. 14 - Prob. 14.7QPCh. 14 - Consider two gas samples at STP: one consisting of...Ch. 14 - Now consider the reaction F2(g)2F(g)at constant...Ch. 14 - Which of the following best describes why entropy...Ch. 14 - Which of the following best explains why entropy...Ch. 14 - How does the entropy of a system change for each...Ch. 14 - How does the entropy of a system change for each...Ch. 14 - Predict whether the entropy change is positive or...Ch. 14 - Prob. 14.11QPCh. 14 - Prob. 14.12QPCh. 14 - Prob. 14.13QPCh. 14 - Using the data in Appendix 2, calculate the...Ch. 14 - Using the data in Appendix 2, calculate the...Ch. 14 - For each pair of substances listed here, choose...Ch. 14 - Arrange the following substances (1 mole each) in...Ch. 14 - State the second law of thermodynamics in words,...Ch. 14 - State the third law of thermodynamics in words,...Ch. 14 - Calculate Ssurr for each of the reactions in...Ch. 14 - Calculate Ssurr for each of the reactions in...Ch. 14 - Using data from Appendix 2, calculate Srxn and...Ch. 14 - Using data from Appendix 2, calculate Srxn and...Ch. 14 - When a folded protein in solution is heated to a...Ch. 14 - Define free energy. What are its units?Ch. 14 - Why is it more convenient to predict the direction...Ch. 14 - What is the significance of the sign of Gsys?Ch. 14 - From the following combinations of H and S,...Ch. 14 - Prob. 14.29QPCh. 14 - Calculate G for the following reactions at 25C....Ch. 14 - Calculate G for the following reactions at 25C....Ch. 14 - From the values of H and S, predict which of the...Ch. 14 - Find the temperatures at which reactions with the...Ch. 14 - The molar heats of fusion and vaporization of...Ch. 14 - The molar heats of fusion and vaporization of...Ch. 14 - Use the values listed in Appendix 2 to calculate G...Ch. 14 - Certain bacteria in the soil obtain the necessary...Ch. 14 - What is a coupled reaction? What is its importance...Ch. 14 - What is the role of ATP in biological reactions?Ch. 14 - Prob. 14.40QPCh. 14 - Predict the signs of H, S, and G of the system for...Ch. 14 - A student placed 1 g of each of three compounds A,...Ch. 14 - The enthalpy change in the denaturation of a...Ch. 14 - Consider the following facts: Water freezes...Ch. 14 - Ammonium nitrate (NH4NO3) dissolves spontaneously...Ch. 14 - The standard enthalpy of formation and the...Ch. 14 - (a) Troutons rule states that the ratio of the...Ch. 14 - Referring to Problem 14.47, explain why the ratio...Ch. 14 - Prob. 14.49QPCh. 14 - Prob. 14.50QPCh. 14 - Prob. 14.51QPCh. 14 - Prob. 14.52QPCh. 14 - Prob. 14.53QPCh. 14 - The molar heat of vaporization of ethanol is 39 3...Ch. 14 - As an approximation, we can assume that proteins...Ch. 14 - When a native protein in solution is heated to a...Ch. 14 - A 74.6-g ice cube floats in the Arctic Sea. The...Ch. 14 - A reaction for which H and S are both negative is...Ch. 14 - The sublimation of carbon dioxide at 78C is given...Ch. 14 - Many hydrocarbons exist as structural isomers,...Ch. 14 - Consider the following reaction at 298 K. 2H2(s) +...Ch. 14 - Which of the following is not accompanied by an...Ch. 14 - Which of the following are not state functions: S,...Ch. 14 - Give a detailed example of each of the following,...Ch. 14 - Hydrogenation reactions (e.g., the process of...Ch. 14 - At 0 K. the entropy of carbon monoxide crystal is...Ch. 14 - Which of the following thermodynamic functions are...Ch. 14 - Using Gf values from Appendix 2, calculate the...Ch. 14 - Prob. 14.2KSPCh. 14 - Using Grxnvalues from Appendix 2, calculate the...Ch. 14 - Prob. 14.4KSP
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- Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)arrow_forward[References] Before two molecules can react, chemists envision that the molecules must first collide with one another. Is collision among molecules the only consideration for the molecules to react with one another? O Yes, collision between molecules is enough for the molecules to react with one another. O Collision between molecules which possess sufficient energy is always enough for the molecules to react with one another. O No, it is not. The molecules must also posses sufficient energy to react, and must have the proper spatial orientation. O Collision is not important. First, the molecules must have the proper spatial orientation. Submit Answer Try Another Version 1 item attempt remainingarrow_forwardAre the processes that move a system toward equilibrium spontaneous or nonspontaneous?arrow_forward
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